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5.1 Monitoring chemical reactions

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Question 10

A chemist uses hydrogen peroxide to make oxygen.

2H2O2(aq)→2H2O(l)+O2(g) 2\mathrm{H_{2}O_{2}(aq)} \rightarrow 2\mathrm{H_{2}O(l)} + \mathrm{O_{2}(g)} 2H2​O2​(aq)→2H2​O(l)+O2​(g)

The chemist starts with 6.80 g of hydrogen peroxide. The percentage yield of oxygen is 70.0%.

The volume of oxygen is measured at room temperature and pressure.

At room temperature and pressure, one mole of any gas occupies 24 dm324\,\mathrm{dm^{3}}24dm3.

Calculate the volume of oxygen collected.

Relative atomic mass (ArA_rAr​): H = 1.0, O = 16.0

Volume = .................... dm3\mathrm{dm^{3}}dm3

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5.1 Monitoring chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /5.1 Monitoring chemical reactions

152 exam-style questions on OCR GCSE Chemistry 5.1 Monitoring chemical reactions, covering 5.1.1 The technique of titration, 5.1.2 Theoretical mass, percentage yield and atom economy, 5.1.3 Concentration of a solution in mol/dm3, 5.1.4 Concentration calculations and titration results, 5.1.5 Molar gas volume and volumes of gases in reactions, and 5.1.6 Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.

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